Section 1
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P orbital
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Last updated
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Date created
Mar 1, 2020
Cards (68)
Section 1
(50 cards)
P orbital
6 electrons
Coulombic attraction
The force of attraction between positive and negative charges (greater distance, weaker attraction)
Increases
As we go down a group, atomic radius and principal quantum number....
Thomson's Plum Pudding Model
dense positive charge with negatively charge electrons interspersed (2nd)
Decreases
As we go from left to right across the table, atomic radius...
F orbital
14 electrons
Bohr Model
model of the atom in which electrons move rapidly around the nucleus in paths called orbits (4th)
Sulfite
SO3 2-
Sulfate
SO4 2-
Hydrogen
A nonmetal, but belongs to no family; reacts with other nonmetals to form molecular (covalent) compounds
SF4
sulfur tetrafluoride
Ionization energy
The minimum energy needed to remove an e- from an atom or ion
Iron(3) chloride
FeCl3
Prefixes are used for...
Covalent
Cathode Ray Experiment
Thomson's experiment where the cathode ray was attracted to a positive magnetic field and repelled by a negative magnetic field (2nd)
NO3-
Nitrate
Larger
Successive ionization energies are larger or smaller than previous ones?: cause we're moving electrons, but the protons stay the same
Alkali metals
The most reactive metals (one e- to lose)
Gold Foil Experiment (Rutherford)
When a beam of alpha particles strikes gold foil, most pass straight through, but some are scattered; the reason for this is presence of a nucleus (3rd)
XeF2
xenon difluoride
Na2SO4
sodium sulfate
Sulfuric acid
H2SO4
S orbital
2 electrons
Change anion suffix from "ate" to...(ternary acid)
Ic
Roman numerals are used for...
Ionic
Ternary acid
oxyacid
Released
For most atoms, adding an e- causes energy to be...released or gained?
NH4+
Ammonium
NO2-
Nitrite
Change anion suffix from "ide" to...(for acid nomenclature)
Ic
Alkaline-earth metals
Not as reactive as alkalis (two e- to lose), harder, denser, and higher melting points
B
Which one takes less ionization energy? Be or B
diphosphorus pentoxide
P2O5
Hund's Rule
Electrons will occupy different orbitals in the same sub level before doubling up in the same orbital
Prefix added to ternary acids...
N/a
CO3 2-
Carbonate
electron affinity
The energy change that occurs when an e- is added to a gaseous atom
More
More (-)e- affinity= more or less willing to accept an e-?
Prefix used for binary acids...
Hydro
Phosphate
PO4 3-
Decreases
As we go down a group, the first Ionization energy... (because more e-/e+ repulsion and shielding)
Halogens
This group has the most (-) electron affinities (they become very stable when they accept electrons)
Increases
Generally, as we go from left to right, 1st Ionization energy...
Dalton's Atomic Theory
Atoms are the smallest particle (1st)
dinitrogen tetroxide
N₂O₄
PtO2
platinum(4) oxide
D orbital
10 electrons
[Ne] 3s2 3p1
Al (aluminum): abbreviated configuration
HCl
hydrochloric acid
Al (aluminum): full electron configuration
1s2 2s2 2p6 3s2 3p1
Section 2
(18 cards)